6.4 LEWIS STRUCTURE DIAGRAMS

LEWIS DIAGRAMS - REVIEW Show only an atom’s valence electrons and the chemical symbol.

LEWIS DIAGRAMS

Rule # 1 Dots representing valence electrons are placed around the element symbols

Rule # 2 Electron dots are placed singly until the fifth electron is reached then they are paired

Lewis Diagrams of IONS and IONIC BONDS For positive ions, one electron dot is removed from the valence shell for each positive charge. For negative ions, one electron dot is added to each valence shell for each negative charge. Square brackets are placed around each ion to indicate transfer of electrons.

LEWIS STRUCTURE DIAGRAMS for MOLECULES Lewis structures are representations of molecules showing all valence electrons: bonding and nonbonding

LEWIS STRUCTURE DIAGRAMS for MOLECULES Lewis structures are representations of molecules showing all valence electrons: bonding and nonbonding a lone pair

Lewis Structures and Multiple Bonds When two electron pairs are shared, two lines are drawn, i.e. double bond ::O :: C :: O:: or ::O = C = O::

Lewis Structures and Multiple Bonds When three electron pairs are shared, three lines are drawn, i.e. triple bond :N ::: N: or :N ≡ N:

N – N N = N N ≡ N BOND LENGTHS > > BOND STRENGTH? The length of the bond between two atoms decreases as the number of shared electrons increases N – N > N = N > N ≡ N BOND STRENGTH?

PCl3 5 + 21 valence electrons = 26 v.e. STEPS TO FOLLOW… Find the sum of valence electrons of all atoms in the polyatomic ion or molecule If it is anion  add an electron(s) If it is cation  subtract an electron(s) PCl3 5 + 21 valence electrons = 26 v.e.

5 + 21 valence electrons = 26 v.e. STEPS TO FOLLOW… 2. Write the symbols for the atoms Make one of the atoms a central atom (usually the least electronegative atom) connect the central atom with the other atoms by single bonds 5 + 21 valence electrons = 26 v.e.

2. Write the symbols for the atoms STEPS TO FOLLOW… 2. Write the symbols for the atoms Subtract the bonding electrons from your total number of valence electrons 5 + 21 valence electrons = 26 v.e.

2. Write the symbols for the atoms STEPS TO FOLLOW… 2. Write the symbols for the atoms Subtract the bonding electrons from your total number of valence electrons 26 – 6 valence electrons = 20 v.e. left

3. Fill the octets of the outer atoms STEPS TO FOLLOW… 3. Fill the octets of the outer atoms 20 valence electrons

3. Fill the octets of the outer atoms STEPS TO FOLLOW… 3. Fill the octets of the outer atoms 20 valence electrons

20 valence electrons STEPS TO FOLLOW… Subtract the added electrons from your total number of valence electrons 20 valence electrons

20 – 18 valence electrons = 2 v.e. left STEPS TO FOLLOW… Subtract the added electrons from your total number of valence electrons 20 – 18 valence electrons = 2 v.e. left

4. Fill the octet of the central atom STEPS TO FOLLOW… 4. Fill the octet of the central atom 2 valence electrons

4. Fill the octet of the central atom STEPS TO FOLLOW… 4. Fill the octet of the central atom 0 valence electrons

Draw Lewis Structures for EXAMPLE Draw Lewis Structures for H2O CH4 CH2Cl2 NH4+

Draw Lewis Structures for WORKSHEET EXAMPLE Draw Lewis Structures for CH2Cl2 C2H4 BrO3-

Draw Lewis Structures for WORKSHEET EXAMPLE Draw Lewis Structures for NO BF3 PF5

EXCEPTIONTS TO THE OCTET RULE 1. For molecules and polyatomic ions containing an odd number of valence electrons 2. For molecules and polyatomic ions in which an atom has fewer than an octet of valence electrons

EXCEPTIONTS TO THE OCTET RULE 3. For molecules and polyatomic ions in which an atom has more than an octet of valence electrons

1. For molecules and polyatomic ions containing an odd number of valence electrons Complete pairing of valence electrons is impossible due to the odd number of valence electrons e.g. ClO2, NO, NO2, O2-

Mostly boron, beryllium, aluminum compounds 2. For molecules and polyatomic ions in which an atom has fewer than an octet of valence electrons Not very common Mostly boron, beryllium, aluminum compounds

WHY? Very common Such molecules/ions are called HYPERVALENT 3. For molecules and polyatomic ions in which an atom has more than an octet of valence electrons Very common Such molecules/ions are called HYPERVALENT Only for atoms of 3rd period or higher WHY? They have available and unfilled d orbitals for bonding 2. Their central atom (P, S, I, Xe…) is large enough to be bonded to even five different smaller atoms (Cl, F or O)

Draw a Lewis structure of carbon dioxide Valence electrons: 16 electrons

Draw a Lewis structure of carbon dioxide 5. If you run out of electrons before the central atom has an octet… …form multiple bonds until it does

Draw a Lewis Structure of hydrogen cyanide 5. If you run out of electrons before the central atom has an octet… …form multiple bonds until it does

HOMEWORK/CLASSWORK 6.4 Review Questions all